1 / 25

Warm up 10-17-13

This lesson covers naming compounds, writing chemical formulas, and drawing Lewis dot structures. It also discusses the formation of ionic bonds and the properties of different types of compounds. Review for upcoming test and complete assignments.

urbano
Download Presentation

Warm up 10-17-13

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Warm up 10-17-13 1. Name the following compounds C2H6 MgCl2 Cu2S Ca(NO3)2 2. Write the chemical formula for these compounds Dinitrogentetraoxide Potassium Oxide Cobalt III Sulfide Agenda -Quiz Chp 4 and 5 -Notes Chp 6 Lewis dot -Practice WS Homework Oct 23 – Test Chp 4, 5 & 6 Oct 24 – Online HW (58)

  2. Review For the Quiz • Chapter 4 – Group names -Trends: radius, electronnegativity ionization energy etc…. • Chapter 5 – Ions (positive and negative charge) - Bonds (3 types)

  3. Chp 6-2Lewis Dot structure How do we determine which elements will combine to make bonds?

  4. G. N. Lewis 1875 - 1946 Electron Distribution in Molecules • Electron distribution is depicted withLewis (electron dot) structures showing valence electrons • This decide how many atoms will bond covalently! (In ionic bonds, it was decided with charges)

  5. Lewis Structures • Write the element symbol. • Carbon is in the 4th group, so it has 4 valence electrons. • Starting at the right, draw 4 electrons, or dots, counter-clockwise around the element symbol. C

  6. Lewis Structures Try these elements on your own: • H • P • Ca • Ar • Cl • Al C

  7. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al H

  8. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al P

  9. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al Ca

  10. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al Ar

  11. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al Cl

  12. Lewis Structures On your worksheet, try these elements on your own: • H • P • Ca • Ar • Cl • Al Al

  13. •• •• Cl H H Cl • • + • • •• •• Bond Formation A bond can result from anoverlapof atomic orbitals on neighboring atoms. •• H Cl • • •• Overlap of H (1s) and Cl (2p) Note that each atom has a single, unpaired electron.

  14. •• H Cl • • •• lone pair (LP) shared or bond pair Bond and Lone Pairs • Valence electrons are distributed as shared orBOND PAIRS and unshared orLONE PAIRS. This is called a LEWIS structure.

  15. Sharing Electrons • All atoms want to have 8 valence electrons (except H, only needs 2) • Obtain a total of 8 by sharing • Example: Cl2 CH4

  16. Bond Formation Single bond - Cl2 Double bond = CO2 Triple bond N2

  17. Compound Lewis Dot Draw carbon dioxide, CO2 Draw Ethylene, C2H4 Draw Hydrogen peroxide H2O2

  18. Warm up 10-17-12 • Name the following compounds: SCl2FeO 2. Write the chemical formula for these compounds diphosphorusdihydride calcium nitride 3. Write the Lewis dot structure for the following: H2S PBr3 C2H2 Agenda -Go over Quiz -Binder Check List -Test Review/Online HW Homework Oct 19 – Test Chp 4, 5 & 6 Oct 20 – Online HW (58) Oct 23 – Binder Check

  19. Quiz Answer 2. This statement is false (not true) adding electron doesn’t always result in the atom getting bigger.When going across the period, the atoms tend to get smaller in size.

  20. Quiz Answer 3. Atoms can gainor lose electrons to become ions (has a charge) 4. Ba2+ P3-

  21. Quiz Answer 5. -Ionic bond = electrons are transferred (one give one take)-Covalent bond = electrons are shared-Metallic bond = sea of electrons, they are free to move around, electrons are able to hop from one atom to another atom (any one of these answer is correct for metallic bond)

  22. Quiz Answer 6. Transferring electrons resulted in a stronger bond thus requiring more energy to break apart.

  23. Chp 4, 5 & 6Binder Due Oct 23

  24. Assignment • Review for Test • Online HW • Complete binder for next week

More Related